Classify each of the following substances as either a strong or weak acid, strong or weak base, or a soluble or insoluble salt.   Clear All H2SO4 KOH CH3COOH PbSO4 NH3   strong acid weak acid strong base weak base soluble salt insoluble salt

Q: How many grams of sodium hydroxide would be required to prepare a 751.0 mL solution of sodium…

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Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

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Q: Classify each of the following salts as a "strong acid-strong base salt," a "strong acid–weak base…

A: Strong acid : Acid which dissociate completely in aqueous solution. ( percent ionization = 100 %)…

Q: substances

A: Weak acid is a weak electrolyte and this will partially dissociated into water and give less amount…

Q: Classify each aqueous solution as acidic, basic, or neutral at 25 °C? Acidic  Basic Neutral Answer…

A: The pH of solution indicates the number of H+ ions in the solution. The pH scale ranges from 0 to 14…

Q: What are the major species present when 10 mL of 0.1 M NaOH are added to 40 mL of 0.05 M acetic acid…

A: When a strong base like NaOH is added to a weak acid like CH3COOH, it undergoes a neutralization…

Q: Place each compound into the appropriate category, based on how the compounds behave in water.…

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Q: Identify the following aqueous salt solutions as acidic, neutral or basic solution. NH4ClO4  LiNO3…

A: 1. NH4ClO4 is acidic since the salt is obtained by the neutralization of weak base and strong acid.…

Q: Calculate the pHpH of each solution. 9.28×10−3 MM KOH 6.89×10−3 MM HNO3 6.54×10−4 MM Sr(OH)2

A: 9.28×10−3 M KOH   6.89×10−3 M HNO3   6.54×10−4 M Sr(OH)2

Q: Which of the following aqueous solutions will be the most conductive They are all equally…

A: The conductivity of an aqueous solution is determined by the number of ions present in the solution.…

Q: Each row of the table below describes an aqueous solution at about 25°C . Complete the table. That…

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Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: To Solve this problem first we have to know about Brønsted–Lowry acid–base theory . According to…

Q: Which graph best represents the titration of sodium hydroxide with hydrochloric acid?

A: In this question, we will select the best curve for the titration between NaOH and HCl. You can see…

Q: HI Ba(OH)2 H3PO4 NH3 NaBr Stan es ds d Clear All strong acid weak acid strong base weak base soluble…

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Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: Since, H3PO4 is a triprotic acid it dissociates with water a follows-

Q: A solution with an H+ concentration of 8.24×10-12 has an OH- concentration of _____.

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Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: Thank you.

Q: The chemical formulae of some acids are listed in the first column of the table below, and in the…

A: The concept used here is from acids and bases of chemistry.  Concept : Strong acids when dissolved…

Q: Three bottles are labelled as shown: Bottle 1 0.001 mol/L HCI(aq) Bottle 2 0.003 mol/L HBr(aq)…

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Q: Sketch two diagrams at the atomic/molecular level for an aqueous solution. Strong Acid Weak Acid

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Q: Which of the following, when combined, is a buffer system? O HCl and KOH H20 and HCl O NaCl and NaOH…

A: In buffer system , a solution that resists a change in pH when acids and bases are added.  Buffer…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

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Q: Determine the [H+] value for solutions with the following characteristics: a pH=9.90 [H+] = bpH =…

A: (a) pH = 9.90 Using the formula we have pH = - log10[H+] [H+] = 10-pH [H+] = 10-9.90 [H+] = 1.26…

Q: Which of the following represents the reaction of the weak base, CH3COO", in water? O CH3COO + H₂O =…

A: The reaction that represents the reaction of the weak base, CH3COO-  in water is

Q: Complete the table by labeling each acid as monoprotic, diprotic, or triprotic. Name of Acid…

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Q: What is the product of a neutralization of hydrosulfuric acid and calcium hydroxide.

A: Hydrosulfuric acid is chemically, H2S

Q: A 25.0-mL sample of a 2.14 M NAOH solution is titrated with a 1.25 M HCI solution. What will be the…

A: The given data contains, Volume of NaOH V1 = 25 ml. Molarity of NaOH M1 = 2.14 M. Volume of HCl V2 =…

Q: QUESTION 6 Identify the salts that will not hydrolyze water. The solution will be neutral. NaCl NH41…

A: Answer:Salts of strong acid and strong base doesn't get hydrolyzed in water. So, in this problem we…

Q: Imagine that a few tenths of a mole of each compound is written in the second columnn of the table.…

A: Ionic compound - These compounds composed of ions when dissolve in water produce ions in solution.…

Q: In the following neutralization reaction, label each compound as the Arrhenius acid Arrhenius base,…

A: According to Arrhenius theory, acid is a substance that gives H+ ion on dissolving in the aqueous…

Q: Classify each of the following substances as either a strong or weak acid, strong or weak base, or a…

A: A substance is said to be a strong acid if it gives easily H+ ions in an aqueous solution. A…

Q: In an aqueous solution, if H* increases then OH decreases. True O False

A: The question is based on the concept of equilibrium. ionic product of water is given as product of…

Q: For the following reaction, K> 1. Classify each of the reactants and products based on their…

A: According to this theory:Bronsted-Lowry acid is a hydrogen ion donor.Bronsted-Lowry base is a…

Q: A typical vitamin C tablet (containing pure ascorbic acid, H₂C6H606) weighs 500 mg. One vitamin C…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: A solution has [H+] = 4.0 x 10-3 M. The [OH"] in this solution is %3D 4.0 x 1011 1.0 x 10 14M 4.0 x…

A: Given data,[H+]=4.0×10-3M

Q: Determine the pHpH of each solution. pOH = 9.7 pOH = 4.8 pOH = 2.5 pOH = 7.0

A: We have given that pOH = 9.7 pOH = 4.8 pOH = 2.5 pOH = 7.0

Q: Which of the following pairs are both weak electrolytes? HCIO4 and NaOH OHCIO4 and NH3 CH3COOH and…

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Q: Which statement is true regarding Kw? 1 [H₂O+][OH The value of Kw is temperature dependent. Kw More…

A: 1. Kw = 1 / [H3O+][OH-]   - This statement is incorrect. Kw is the ion product of water and is equal…

Q: Use the graph to show the change in concentration when:  a persons blood pH change if they were…

A: We must take into account the processes involving CO2  , H2O, H2CO3, H+, and HCO3- in order to…

Q: Which of these species can function as a weak base in solution? CHBrClF (bromochlorofluoromethane)…

A: Given: 1.CHBrClF, 2.NH(CH3)3Cl 3.Li2HPO4 among all the given compounds, .NH(CH3)3Cl is a strong base…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.